(a)
Interpretation:
The equilibrium concentrations of H+ and CH3 COO- have to be determined given the initial concentration and final concentration of the weak acid, CH3 COOH.
Concept Introduction:
Answer to Problem 53P
Explanation of Solution
The equilibrium reaction representing the ionization of weak acid,
The initial concentration of the acid = 0.10 M.
Concentration of acid at equilibrium = 0.098 M.
Change in concentration of
This change in concentration of CH3 COOH will be equal to the concentration of
Therefore,
(b)
Interpretation:
The expected equilibrium constant for the above reaction has to be calculated.
Concept Introduction:
Equilibrium constant is the ratio of the concentrations of products to the reactants concentrations, each term raised to the power equal to the
Answer to Problem 53P
The expected equilibrium constant for the reaction is
Explanation of Solution
The given equilibrium ionization reaction is,
Plugging in the equilibrium concentrations to calculate the K value,
Want to see more full solutions like this?
Chapter 7 Solutions
Introduction To General, Organic, And Biochemistry
- Write equilibrium constant expressions for the following generalized reactions. a. 2X(g)+3Y(g)2Z(g) b. 2X(g)+3Y(s)2Z(g) c. 2X(s)+3Y(s)2Z(g) d. 2X(g)+3Y(g)2Z(s)arrow_forwardWrite a balanced chemical equation for a totally gaseous equilibrium system that would lead to the following equilibrium constant expression. Keq=[N2]2[H2O]6[NH3]4[O2]3arrow_forward7-40 Is there any change in conditions that change the equilibrium constant, K, of a given reaction?arrow_forward
- 7-22 If you add a piece of marble, CaCO3 to a 6 M HCI solution at room temperature, you will see some bubbles form around the marble as gas slowly rises. If you crush another piece of marble and add it to the same solution at the same temperature, you will see vigorous gas formation, so much so that the solution appears to be boiling. Explain.arrow_forwardSuppose a reaction has the equilibrium constant K = 1.3 108. What does the magnitude of this constant tell you about the relative concentrations of products and reactants that will be present once equilibrium is reached? Is this reaction likely to be a good source of the products?arrow_forward. What does it mean to say that a state of chemical or physical equilibrium is dynamic?arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage LearningChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
- Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning